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Transcript of Metals and Metal Compounds Unit E. Do Now: What characteristics does a metal have? What is an...
Metals and Metal Compounds
Unit E
Do Now:
• What characteristics does a metal have?• What is an example of a metal?
Metals
• Periodic Table – contains all elements• Elements – a substance made of 1 type of
atom• Metal – an element that is usually a good
conductor– Contains physical and chemical properties
How do you tell if it is a metal?
• Physical Properties– Malleability, conductive, colour, sonorous, melting
point, boiling point
• Chemical Properties– A reaction with another substance, ex. Iron rusting
The Periodic Table
Types of Metals – Group 1
• Alkali Metals – very reactive, usually found combined with another substance
Group 2
• Alkaline Earth Metals – Reactive, harder than alkali metals, usually combined with other elements
Groups 3-12
• Transition Metals – most common metals, good conductors of electricity. Hard and shiny
Other metal groups:
• Metalloids• Lanthanides• Actinides• Post – Transition Metals
Do Now:
• Name each of the following and classify what type of metal it is:– Mg– Al– Cs– Fe– Sn– Ge
Making Salts
• Salt – A substance produced when an acid reacts with a base– Sulphates– Chlorides– Nitrates
What is an ACID?
• pH less than 7• Neutralizes bases• Forms H + ions in solution• Corrosive-reacts with most metals to form
hydrogen gas• Good conductors of electricity
Common Acids
• HCl- hydrochloric- stomach acid• H2SO4- sulfuric acid - car batteries
• HNO3 – nitric acid - explosives
• HC2H3O2- acetic acid - vinegar
• H2CO3-carbonic acid – sodas
• H3PO4- phosphoric acid -flavorings
What is a BASE?
• pH greater than 7• Feels slippery• Dissolves fats and oils• Usually forms OH- ions in solution• Neutralizes acids
Weak vs. Strong Bases
• Weak Bases: ammonia; potassium carbonate, sodium carbonate
• Strong Bases: sodium hydroxide; sodium phosphate; barium hydroxide; calcium hydroxide
Common Bases
• NaOH- sodium hydroxide (LYE) soaps, drain cleaner
• Mg (OH)2 - magnesium hydroxide-antacids
• Al(OH)3-aluminum hydroxide-antacids, deodorants
• NH4OH-ammonium hydroxide- “ammonia”
What is a SALT?
• A salt is a neutral substance produced from the reaction of an acid and a base.
• Composed of the negative ion of an acid and the positive ion of a base.
• One of the products of a Neutralization Reaction
• Examples: KCl, MgSO4, NaNO2
Metal + Acid = A Salt
• Mg + HCl →• Zn + HCl → • Fe + HCl →• Sn + HCl →• Cu + HCl →
Write out the equations
Do Now:
• Answer questions a-d on page 64
Acids and Bases
• Pure metal + acid = salt + hydrogen gas
• Base + Acid = salt + water–Bases are a metal with:• Oxides• Hydroxides• Carbonates
Identify the following:
• MgO• HNO3
• KOH
• Ca(OH)2
• HCl
• NaOH • CaCO3
Name the following:
• HNO3
• KOH
• Ca(OH)2
• HCl
• NaOH • MgO• CaCO3
Neutralization
• Neutralization – Reaction between an acid and a base.
• What is the pH of a base?• What is the pH of an acid?• What is the pH after neutralization?
Reactions
• Acid + metal oxide → a salt + water• Acid + metal hydroxide → a salt + water• Acid + metal carbonate → a salt + water + carbon dioxide
• https://phet.colorado.edu/en/simulation/concentration
Properties of Acids:
• they taste sour• turn litmus paper red• react with certain metals to yield hydrogen
gas.
Properties of Bases:
• they taste bitter• turn litmus paper blue• feel slippery
Common Acids and Bases at Home:
• Vinegar• Baking soda• Soap• Ammonia • Soda• http://
www.ehow.com/list_6930749_acids-bases-found-homes.html
Do Now:
• Look at your results from yesterdays titration lab. Compare your acid and base. Which is stronger or are they similar?
• Why?
Need to Know Chemical Formulas:
• Products:– Water H2O
– Hydrogen Gas H2
– Carbon Dioxide CO2
• Acids:– Hydrochloric Acid HCl– Sulphuric Acid H2SO4
– Nitric Acid HNO3
Reactions with a Metal:
• Hydrochloric Acid + Metal → Metal chloride + hydrogen gas
• Sulphuric Acid + Metal → Metal sulphate + hydrogen gas
• Nitric Acid + Metal → Metal Nitrate + hydrogen gas
Reactions with Metal Oxides:• Hydrochloric Acid +Metal Oxide → Metal Chloride + Water • Sulphuric Acid + Metal Oxide → Metal Sulphate + Water• Nitric Acid + Metal Oxide → Metal Nitrate + Water
• Oxide = Metal and only oxygen– MgO– Na2O
– Al2O3
Reactions with Metal Hydroxides:
• Hydrochloric Acid + Metal Hydroxide → Metal Chloride + Water • Sulphuric Acid + Metal Hydroxide → Metal Sulphate + Water• Nitric Acid + Metal Hydroxide → Metal Nitrate + Water
• The biggest change with a hydroxide from an oxide, the final equation WILL need to balanced!
• Metal Hydroxide = Metal with an oxygen and hydrogen (OH)– NaOH– Al(OH)3
– Ba(OH)2
Reactions with Metal Carbonates:• Hydrochloric Acid + Metal Carbonate → Metal Chloride + Water + Carbon Dioxide• Sulphuric Acid + Metal Carbonate → Metal Sulphate + Water + Carbon Dioxide• Nitric Acid + Metal Carbonate → Metal Nitrate + Water + Carbon Dioxide
• Carbonates will ALWAYS produce carbon dioxide!• These reactions will usually need to be balanced!
• Metal Carbonate = Metal with carbon and oxygen (CO3)
– CaCO3
– MgCO3
– Na2CO3
Activity:
• Complete the worksheet for practice
Do Now:
• Complete and balance the following reactions:1. _____ + NaOH → NaCl + ________2. H2SO4 + Al2(CO3)3 → Al2(SO4)3 + ___________
3. _______ + Zn → Zn(NO3)2 + ____________
4. HCl + _________ → KCl + H2
5. ______ + Ba(OH)2 → Ba(NO3)2 + __________
Use of Salts
• Sodium Chloride – table salt
Fertilizers
• Fertilizer – Nutrients that can be added to a soil if needed–Many are made up of :• Nitrogen (N)• Phosphorus (P)• Potassium (K)
NPK
• Fertilizers often have 3 numbers, representing the percentage of each element inside
NPK
• Nitrogen provides plants with the ability to produce more chlorophyll, which in turn allows plants to grow quickly
• Phosphorous aids in root development and increases flowering ability and bloom size
• Potassium has many functions:– It guards the plant against diseases – Aids in drought protection and cold tolerance. – Serves a role in improving root development– helps in the process of photosynthesis
How much of each?
• Why is the total percent not 100?
Activity:
• Open your books to page 67:• Answer questions 1 and 2• Besides, fertilizers and table salt, what other
places do you see salts being used?